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The number of monomers in the polymer can be determined from the molar mass of the polymer and monomer from the relationship: Number of monomers/repeating units in monomer = Molar mass polymer Molar mass monomer Examples Polythene has a molar mass of 4760.Calculate the number of ethene molecules in the polymer(C=12.0, ... | {
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It is an elastic, tough, transparent and durable plastic. Polythene is used: (i)in making plastic bag (ii)bowls and plastic bags (iii)packaging materials
106 2.Formation of Polychlorethene Polychloroethene is an addition polymer formed when chloroethene molecule/monomer join together to form a large molecule/polymer at... | {
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Polythene is used: (i)in making plastic bag (ii)bowls and plastic bags (iii)packaging materials
106 2.Formation of Polychlorethene Polychloroethene is an addition polymer formed when chloroethene molecule/monomer join together to form a large molecule/polymer at high temperatures and pressure. During polymerization: (i... | {
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During polymerization: (i)many molecules are brought nearer to each other by the high pressure(which reduces the volume occupied by reacting particles) H H H H H H H H C = C + C = C + C = C + C = C + β¦ H Cl H Cl H Cl H Cl chloroethene + chloroethene + chloroethene + chloroethene + β¦ (ii)the double bond joining the chlo... | {
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Polychloroethene molecule can be represented as: H H H H H H H H extension of molecule/polymer - C β C - C β C - C β C - C β C- + β¦
107 H Cl H Cl H Cl H Cl Since the molecule is a repetition of one monomer, then the polymer is: H H ( C β C )n H Cl Examples Polychlorothene has a molar mass of 4760.Calculate the number o... | {
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It is a tough, non-transparent and durable plastic. PVC is used: (i)in making plastic rope (ii)water pipes (iii)crates and boxes 3.Formation of Polyphenylethene Polyphenylethene is an addition polymer formed when phenylethene molecule/monomer join together to form a large molecule/polymer at high temperatures and press... | {
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PVC is used: (i)in making plastic rope (ii)water pipes (iii)crates and boxes 3.Formation of Polyphenylethene Polyphenylethene is an addition polymer formed when phenylethene molecule/monomer join together to form a large molecule/polymer at high temperatures and pressure. During polymerization: (i)many molecules are br... | {
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During polymerization: (i)many molecules are brought nearer to each other by the high pressure(which reduces the volume occupied by reacting particles) H H H H H H H H C = C + C = C + C = C + C = C + β¦ H C6H5 H C6H5 H C6H5 H C6H5 phenylethene + phenylethene + phenylethene + phenylethene + β¦
108 (ii)the double bond join... | {
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Polyphenylethene molecule can be represented as: H H H H H H H H - C β C - C β C - C β C - C - C - H C6H5 H C6H5 H C6H5 H C6H5 Since the molecule is a repetition of one monomer, then the polymer is: H H ( C β C )n H C6H5 Examples Polyphenylthene has a molar mass of 4760.Calculate the number of phenylethene molecules in... | {
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It is a very light durable plastic. Polystyrene is used: (i)in making packaging material for carrying delicate items like computers, radion,calculators. (ii)ceiling tiles (iii)clothe linings 4.Formation of Polypropene Polypropene is an addition polymer formed when propene molecule/monomer join together to form a large ... | {
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During polymerization: (i)many molecules are brought nearer to each other by the high pressure(which reduces the volume occupied by reacting particles) H H H H H H H H C = C + C = C + C = C + C = C + β¦ H CH3 H CH3 H CH3 H CH3 propene + propene + propene + propene + β¦ (ii)the double bond joining the phenylethene molecul... | {
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It is a very light durable plastic. Polystyrene is used: (i)in making packaging material for carrying delicate items like computers, radion,calculators. (ii)ceiling tiles (iii)clothe linings 5.Formation of Polytetrafluorothene Polytetrafluorothene is an addition polymer formed when tetrafluoroethene molecule/monomer jo... | {
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Polystyrene is used: (i)in making packaging material for carrying delicate items like computers, radion,calculators. (ii)ceiling tiles (iii)clothe linings 5.Formation of Polytetrafluorothene Polytetrafluorothene is an addition polymer formed when tetrafluoroethene molecule/monomer join together to form a large molecule... | {
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(ii)ceiling tiles (iii)clothe linings 5.Formation of Polytetrafluorothene Polytetrafluorothene is an addition polymer formed when tetrafluoroethene molecule/monomer join together to form a large molecule/polymer at high temperatures and pressure. During polymerization: (i)many molecules are brought nearer to each other... | {
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During polymerization: (i)many molecules are brought nearer to each other by the high pressure(which reduces the volume occupied by reacting particles) F F F F F F F F
111 C = C + C = C + C = C + C = C + β¦ F F F F F F F F tetrafluoroethene + tetrafluoroethene+ tetrafluoroethene+ tetrafluoroethene + β¦ (ii)the double bon... | {
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polytetrafluoroethene molecule can be represented as: F F F F F F F F extension of molecule/polymer - C β C - C β C - C β C - C β C- + β¦ F F F F F F F F Since the molecule is a repetition of one monomer, then the polymer is: F F ( C β C )n F F Examples
112 Polytetrafluorothene has a molar mass of 4760.Calculate the num... | {
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The latex is then added an acid to coagulate the rubber. Natural rubber is a polymer of 2-methylbut-1,3-diene ; H CH3 H H CH2=C (CH3) CH = CH2 H - C = C β C = C - H During natural polymerization to rubber, one double C=C bond break to self add to another molecule.The double bond remaining move to carbon β2β thus; H CH3... | {
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6.Formation of synthetic rubber Synthetic rubber is able to resist action of oil,abrasion and organic solvents which rubber cannot. Common synthetic rubber is a polymer of 2-chlorobut-1,3-diene ; H Cl H H CH2=C (Cl CH = CH2 H - C = C β C = C - H During polymerization to synthetic rubber, one double C=C bond is broken t... | {
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(ii)monomers realign themselves at the functional group. (iii)from each functional group an element is removed so as to form simple molecule (of usually H2O/HCl) (iv)the two monomers join without the simple molecule of H2O/HCl Examples of condensation polymerization 1.Formation of Nylon-6,6 Method 1: Nylon-6,6 can be m... | {
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Polymer bond linkage Nylon-6,6 derive its name from the two monomers each with six carbon chain Method 2: Nylon-6,6 can be made from the condensation polymerization of hexan1,6-dioyl dichloride with hexan-1,6-diamine. Hexan-1,6-dioyl dichloride belong to a group of homologous series with a general formula R-OCl and thu... | {
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2.Formation of Terylene
116 Method 1: Terylene can be made from the condensation polymerization of ethan1,2-diol with benzene-1,4-dicarboxylic acid. Benzene-1,4-dicarboxylic acid a group of homologous series with a general formula R-COOH where R is a ring of six carbon atom called Benzene ring .The functional group is ... | {
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O O Cl - C β C5H5 β C β Cl + H βO β CH2 CH2 β O - H (iii)from each functional group an element is removed so as to form a molecule of HCl and the two monomers join at the linkage . O O Cl - C β C5H5 β C β O β CH2 CH2 β O β H + HCl . Polymer bond linkage of terylene
118 The commercial name of terylene is Polyester /poly... | {
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(C = 12; H = 1; N = 14; O =16) 7. The formula below represents active ingredients of two cleansing agents A and B O CH3CH2CH C OH
121 Which one of the cleansing agents would be suitable to be used in water containing magnesium hydrogen carbonate? Explain
122 8. Study the polymer below and use it to answer the questions... | {
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(a) (i) The table below shows the volume of oxygen obtained per unit time when hydrogen peroxide was decomposed in the presence of manganese (IV) Oxide. Use it to answer the questions that follow:- Time in seconds Volume of Oxygen evolved (cm3) 0 30 60 90 120 150 180 210 240 270 300 0 10 19 27 34 38 43 45 45 45 45 (i) ... | {
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(ii) Write the equation of a reaction that occurs at the cathode
125 (iii) Calculate the mass of Zinc that is consumed when a current of 0.1amperes flows through the above cell for 30minutes (1F =96500c Zn =65) 12. (a) Give the IUPAC names of the following compounds: (i) CH3COOCH2CH3 * (ii) (b) The structure below show... | {
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(II) If the relative molecular mass of U is 42000, determine the value of n (C=12, H=1) (c) State why C2H4 burns with a more smoky flame than C2H6 * 13. a) State two factors that affect the properties of a polymer b) Name the compound with the formula below : CH3CH2CH2ONa c) Study the scheme below and use it to answer ... | {
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(d) A sample of polymer Q is found to have a molecular mass of 4200. Determine the number of monomers in the polymer (H = 1, C = 12) (e) Name the type of reaction in step I β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦.. (f) State one industrial application of step III (g)State how burning can be used to distinguish between propane and propy... | {
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Lβ¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦.. M KMnO4/H+ CH2CH2 Ethyl Ethanoate CH2CH2OH L J K CO2 (g) STEP 2 Reagent Q St3KMnO4/H+(aq) Ni/H2(g) Step 4 Reagent P
132 Products C2H5COONa Step V ClbiCH οΊCH Step I Step II CH2 = CH2 Step III C2H6 Step IV + Heat (ii) Name the process in step: Step 2 β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦β¦.β¦. Step 4 β¦β¦β¦β¦β¦β¦β¦β¦β¦... | {
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Calculate the concentration of the resulting salt solution in moles per litre. (Given that the molecula mass of the salt is 278) 20. Write an equation to show products formed for the complete combustion of CH = CH
134 iii) Explain one disadvantage of continued use of items made form the compound formed in step III
135 ... | {
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Ethanol B Ethanoic acid Na2CO3 Salt A + CO2 + H2O
137 (b) Draw the structural formulae of two compounds that may be reacted to form ethylpropanoate 27. (a) Draw the structure of pentanoic acid (b) Draw the structure and give the name of the organic compound formed when ethanol reacts with pentanoic acid in presence of ... | {
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(b) Explain why plastics and rubbers are used this way
141 32. The scheme below represents the manufacture of a cleaning agent X (a) Draw the structure of X and state the type of cleaning agent to which X belong (b) State one disadvantage of using X as a cleaning agent 33. Y grams of a radioactive isotope take 120days ... | {
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It has molecular formula N2. It has atomic number 7 and atomic weight 14.08 and its electronic configuration of 2,5. Besides combining with hydrogen and forming NH3 , nitrogen combines with oxygen in different ratios and forms five different oxides. The oxides of nitrogen and the details of the oxygen states of nitroge... | {
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Physical Properties: NO is not a combustible gas. At high temperature around 1000Β°C it decomposes into N2 and O2 . 2NO = N2 + O2 at high temperature From the equation above we can see that once the decomposition starts 50% O2 gets evolved and this O2 supports combustion thus making the reaction more violent. Chemical p... | {
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2) It does not support combustion. 3) It is not combustible. Chemical Properties: 1) With cold water NO2 reacts to give a mixture of HNO2 and HNO3 acid. 2NO2 + H2O β HNO2 + HNO3 2) With hot water the reaction is 3NO2 + H2O β 2HNO3 + NO 3) Being acidic it reacts with bases as 2NO2 + KOH β KNO3 + H2O + KNO2 4) It is also... | {
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2) Unlike other oxides of nitrogen, N2O supports combustion though it does not burn itself. Chemical Properties: 1) At very high temperature N2O decomposes to N2 and O2 2N2O β 2N2 + O2 If a glowing piece of Mg, Cu, or P is introduced in such an environment, these pieces burn brightly due to the O2 produced from decompo... | {
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Superheated water at 170oC and 10atmosphere pressure is forced through the outermost pipe. The high pressures ensure the water remains as liquid at high temperatures instead of vapour of vapour /gas. The superheated water melts the sulphur because the melting point of sulphur is lower at about at about 115oC. A compres... | {
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D. Heating Sulphur. A molecule of sulphur exists as puckered ring of eight atoms joined by covalent bonds as S8. On heating the yellow sulphur powder melts at 113oC to clear amber liquid with low viscosity and thus flows easily. On further heating to 160oC the molten liquid darkens to a brown very viscous liquid that d... | {
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Moist/damp/wet blue and red litmus papers were put in a gas jar containing air/oxygen. Burning sulphur was then lowered into the gas jar. State and explain the observation made. Observations -Sulphur melts then burns with a blue flame Colourless gas produced that has a pungent smell Red litmus paper remains red. Blue l... | {
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When a mixture of iron and sulphur is heated, the reaction is exothermic giving out heat energy that makes the mixture to continue glowing even after stopping heating. Black Iron(II)sulphide is formed which is a compound and thus not ferromagnetic. Chemical equation Fe(s) + S(s) -> FeS(s) (Exothermic reaction/ -βH) Hea... | {
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5.State three main uses of sulphur . Sulphur is mainly used in: (i)Contact process for the manufacture/industrial/large scale production of concentrated sulphuric(VI)acid. (ii)Vulcanization of rubber to make it harder, tougher, stronger, and more durable. (iii)Making gun powder and match stick heads (iv) As ointments t... | {
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Monoclinic sulphur B . Rhombic sulphur III. State two main uses of sulphur. -Manufacture of sulphuric(VI)acid -as fungicide -in vulcanization of rubber to make it harder/tougher/ stronger -manufacture of dyes /fibres L M N
9 (d)Calculate the volume of sulphur (IV)oxide produced when 0.4 g of sulphur is completely burnt... | {
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(iii) Sulphuric(VI)acid (iv) Hydrogen Sulphide (v) Sulphate(IV)/SO32- and Sulphate(VI)/ SO42- salts (i) Sulphur(IV)oxide(SO2) (a) Occurrence Sulphur (IV)oxide is found in volcanic areas as a gas or dissolved in water from geysersand hot springs in active volcanic areas of the world e.g. Olkaria and Hells gate near Naiv... | {
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Method 2:Using Sodium Sulphate(IV) and hydrochloric acid. 11 (c)Properties of Sulphur(IV)oxide(Questions) 1. Write the equations for the reaction for the formation of sulphur (IV)oxide using: (i)Method 1 Cu(s) + 2H2SO4(l) -> CuSO4(aq) + SO2(g) + 2H2O(l) Zn(s) + 2H2SO4(l) -> ZnSO4(aq) + SO2(g) + 2H2O(l) Mg(s) + 2H2SO4(l... | {
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3. The diagram below show the solubility of sulphur (IV)oxide gas. Explain. Sulphur(IV) oxide is very soluble in water. One drop of water dissolves all the Sulphur (IV) oxide in the flask leaving a vacuum. If the clip is removed, atmospheric pressure forces the water up through the narrow tube to form a fountain to occ... | {
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Weak sulphuric(IV)acid(H2 SO3 (aq)) dissociates /ionizes into free H+(aq)ions: H2 SO3 (aq) -> 2H+(aq) + SO32- (aq) The free H+(aq)ions are responsible for turning blue litmus paper turns red showing the gas is acidic. The SO32- (aq) ions in wet/damp/moist sulphur(IV) oxide gas is responsible for many reactions of the g... | {
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Old newspapers turn brown on exposure to air on regaining the atomic oxygen. The bleaching through adding oxygen by chlorine gas is permanent. (b)Turns Orange acidified potassium dichromate(VI) to green Experiment: (i)Pass a stream of Sulphur(IV) oxide gas in a test tube containing acidified potassium dichromate(VI) so... | {
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Hydrogen sulphide also reduces acidified potassium dichromate(VI) from orange Cr2O72- ions to green Cr3+ ions leaving a yellow residue. (c)Decolorizes acidified potassium manganate(VII)
15 Experiment: (i)Pass a stream of Sulphur(IV) oxide gas in a test tube containing acidified potassium manganate(VII) solution. or; (i... | {
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(d)Decolorizes bromine water Experiment: (i)Pass a stream of Sulphur(IV) oxide gas in a test tube containing bromine water . or; (ii)Put three drops of bromine water into a gas jar containing Sulphur(IV) oxide gas. Swirl. Observation: Yellow bromine water turns to colourless/ bromine water is decolorized. Explanation:
... | {
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(e)Reduces Iron(III) Fe3+ salts to Iron(II) salts Fe2+ Experiment: (i)Pass a stream of Sulphur(IV) oxide gas in a test tube containing about 3 cm3 of Iron (III)chloride solution. or; (ii)Place about 3cm3 of Iron (III)chloride solution into a gas jar containing Sulphur(IV) oxide gas.Swirl. Observation: Yellow/brown Iron... | {
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Swirl. Observation: Brown fumes of a gas evolved/produced. Explanation: Sulphur(IV) oxide gas reduces concentrated nitric(V)acid to brown nitrogen(IV)oxide gas itself oxidized from SO32- ions in sulphuric(IV) acid to SO42- ions in sulphuric(VI) acid. Chemical/ionic equation: SO2(g) + 2HNO3 (l) -> H2 SO4 (l) + NO2 (g) (... | {
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Chemical/ionic equation: SO32-(aq) + Ba2+ (aq) -> BaSO3(s) white precipitate SO42-(aq) + Ba2+ (aq) -> BaSO4(s) white precipitate CO32-(aq) + Ba2+ (aq) -> BaCO3(s) white precipitate
18 If nitric(V)/hydrochloric acid is added to the three suspected insoluble white precipitates above, the white precipitate: (i) persist/re... | {
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Magnesium burns to produce enough heat energy to decompose Sulphur(IV)oxide to sulphur and oxygen. The metal continues to burn on Oxygen forming white Magnesium oxide solid/ash. Yellow specks of sulphur residue form on the sides of reaction flask/gas jar. During the reaction, Sulphur(IV)oxide is reduced(oxidizing agent... | {
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(i)In the contact process for the manufacture of Sulphuric(VI)acid (ii)As a bleaching agent of pulp and paper. (iii)As a fungicide to kill microbesβ (iv)As a preservative of jam, juices to prevent fermentation (ii) Sulphur(VI)oxide(SO3) (a) Occurrence Sulphur (VI)oxide is does not occur free in nature/atmosphere (b) Pr... | {
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Chemical equation FeSO4.7H2O(s) -> FeSO4(s) + 7H2O(l) (green solid) (white solid) On further heating ,the white anhydrous Iron(II)sulphate(VI) solid decomposes to a mixture of Sulphur (VI)oxide and Sulphur (IV)oxide gas. Sulphur (VI) oxide readily / easily solidify as white silky needles when the mixture is passed thro... | {
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Raw materials The main raw materials for industrial preparation of Sulphuric(VI)acid include: (i)Sulphur from Fraschs process or from heating metal sulphide ore like Galena(PbS),Zinc blende(ZnS) (ii)Oxygen from fractional distillation of air (iii)Water from rivers/lakes II. Chemical processes The contact process involv... | {
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22 (ii)Purification of Sulphur(IV)oxide Sulphur(IV)oxide gas contain dust particles and Arsenic(IV)oxide as impurities. These impurities βpoisonβ/impair the catalyst by adhering on/covering its surface. The impurities are removed by electrostatic precipitation method . In the contact process Platinum or Vanadium(V)oxid... | {
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(iv)Conversion of Sulphur(VI)oxide of Sulphuric(VI)acid Sulphur(VI)oxide is the acid anhydride of concentrated Sulphuric(VI)acid. Sulphur(VI)oxide reacts with water to form thick mist of fine droplets of very/highly corrosive concentrated Sulphuric(VI)acid because the reaction is highly exothermic. To prevent this, Sul... | {
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This prevents the formation of fine droplets of the corrosive/ toxic/poisonous fumes of concentrated sulphuric (VI) acid. (iii)scrubbing-This involves passing the exhaust gases through very tall chimneys lined with quicklime/calcium hydroxide solid. This reacts with Sulphur (VI)oxide gas forming harmless calcium(II)sul... | {
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(v)The following are some chemical properties of concentrated sulphuric (VI) acid: I. As a dehydrating agent Experiment I; Put about four spatula end fulls of brown sugar and glucose in separate 10cm3 beaker. Carefully add about 10cm3 of concentrated sulphuric (VI) acid .Allow to stand for about 10 minutes. Observation... | {
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Explanation Concentrated sulphuric (VI) acid is strong dehydrating agent.It removes physically combined elements of water(Hydrogen and Oxygen in ratio 2:1)from hydrated compounds. The acid dehydrates blue copper(II)sulphate to white anhydrous copper(II)sulphate . Chemical equation CuSO4.5H2O(s) --conc.H2SO4--> CuSO4 (s... | {
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Explanation Concentrated sulphuric (VI) acid is strong dehydrating agent. It removes chemically combined elements of water (Hydrogen and Oxygen in ratio 2:1)from compounds. The acid dehydrates methanoic acid to poisonous/toxic carbon(II)oxide gas. Chemical equation HCOOH(l) --conc.H2SO4 --> CO(g) + H2O(l) NB: This reac... | {
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Put about 0.5g of Copper turnings, Zinc granule and Iron filings to each boiling tube separately. Observation; Effervescence/fizzing/bubbles Blue solution formed with copper, Green solution formed with Iron Colourless solution formed with Zinc Colourless gas produced that has a pungent irritating choking smell. Gas pro... | {
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Gas produced turn orange moist/damp/wet filter paper dipped in acidified potassium dichromate (VI)solution to green. Explanation Concentrated sulphuric (VI) acid is strong oxidizing agent. It oxidizes nonmetals to non metallic oxides and itself reduced to sulphur(IV)oxide gas. Sulphur (IV) oxide gas turn orange moist/d... | {
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(i)Chemical equation KNO3(s) + H2SO4(aq) --> KHSO4(l) + HNO3(g) NaNO3(s) + H2SO4(aq) --> NaHSO4(l) + HNO3(g)
29 This reaction is used in the school laboratory preparation of Nitric(V) acid (HNO3). (ii)Chemical equation KCl(s) + H2SO4(aq) --> KHSO4(s) + HCl(g) NaCl(s) + H2SO4(aq) --> NaHSO4(s) + HCl(g) This reaction is ... | {
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Cover the mixture with a finger as stopper. Introduce a burning splint on top of the finger and release the finger βstopperβ. Repeat by adding Zinc, Copper and Iron instead of the Magnesium ribbon. Observation: No effervescence/ bubbles/ fizzing with copper Effervescence/ bubbles/ fizzing with Iron ,Zinc and Magnesium ... | {
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When a metal lower than hydrogen in the reactivity/electrochemical series is put in a test tube containing dilute sulphuric(VI)acid, there is no effervescence/ bubbling/ fizzing that take place. Copper thus do not react with dilute sulphuric(VI)acid. Chemical/ionic equation Mg(s) + H2SO4(aq) --> MgSO4(aq) + H2(g) Mg(s)... | {
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Green solution formed with Iron(II)Carbonate Blue solution formed with Copper(II)Carbonate Explanation: When a metal carbonate or a hydrogen carbonates is put in a test tube containing dilute sulphuric(VI)acid, effervescence/ bubbling/ fizzing takes place with evolution of carbon(IV)oxide gas. carbon(IV)oxide gas
31 ex... | {
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(v)Neutralization-reaction of metal oxides and alkalis/bases Experiment I: Place 5cm3 of 0.2M dilute sulphuric(VI)acid into four separate clean boiling tubes. Add about 0.1g of copper(II)oxide to one boiling tube. Stir. Repeat by adding Zinc oxide, calcium carbonate and Sodium (II)Oxide in place of the Copper(II)Oxide.... | {
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Chemical/ionic equation ZnO(s) + H2SO4(aq) --> ZnSO4(aq) + H2O(l) ZnO(s) + 2H+(aq) --> Zn2+ (aq) + H2O(l)
32 CuO(s) + H2SO4(aq) --> CuSO4(aq) + H2O(l) CuO(s) + 2H+(aq) --> Cu2+ (aq) + H2O(l) MgO(s) + H2SO4(aq) --> MgSO4(aq) + H2O(l) MgO(s) + 2H+(aq) --> Mg2+ (aq) + H2O(l) Na2O(s) + H2SO4(aq) --> Na2SO4(aq) + H2O(l) Na2... | {
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Pipette 20.0cm3 of 0.1Msodium hydroxide solution into a 250cm3 conical flask. Add three drops of phenolphthalein indicator.Titrate the acid to get a permanent colour change.Repeat with0.1M potassium hydroxide solution inplace of 0.1Msodium hydroxide solution Observation: Colour of phenolphthalein changes from pink to c... | {
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State three physical properties unique to Hydrogen sulphide. Hydrogen sulphide is a colourless gas with characteristic pungent poisonous smell of rotten eggs. It is soluble in cold water but insoluble in warm water. It is denser than water and turns blue litmus paper red. 3. Hydrogen sulphide exist as a dibasic acid wh... | {
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Hydrogen sulphide gas blackens moist Lead (II) ethanoate /Lead (II) nitrate(V) paper . The gas reacts with Pb2+ in the paper to form black Lead(II)sulphide. This is the chemical test for the presence of H2S other than the physical smell of rotten eggs. Chemical equations Pb2+(aq) + H2S -> PbS + 2H+(aq) (black) Fe2+(aq)... | {
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Observation: Orange acidified potassium dichromate (VI) turns to green. Yellow solid residue. Explanation: Hydrogen sulphide gas reduces acidified potassium dichromate(VI) from orange Cr2O72- ions to green Cr3+ ions leaving a yellow solid residue as itself is oxidized to sulphur. Chemical/ionic equation: 4H2S(aq) + Cr2... | {
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Chemical/ionic equation: 5H2S(g) + 2MnO4- (aq) +6H+(aq) -> 5S (s) + 2Mn2+(aq) + 8H2O(l) (purple) (colourless) This is another test for differentiating Hydrogen sulphide and Sulphur(IV) oxide gas. Sulphur(IV) oxide also decolorizes acidified potassium manganate(VII) from purple MnO4- ions to colourless Mn2+ ions leaving... | {
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Swirl. Observation: Yellow/brown Iron (III)chloride solution turns to green. Yellow solid solid Explanation: Hydrogen sulphide gas reduces Iron (III)chloride solution from yellow/brown Fe3+ ions to green Fe2+ ions leaving a yellow residue.The gas is itself oxidized to sulphur. Chemical/ionic equation: H2S(aq) + 2Fe3+ (... | {
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Swirl. Observation: Yellow solid residue Explanation: Hydrogen sulphide gas reduces concentrated sulphuric(VI)acid to yellow sulphur. Chemical/ionic equation: 3H2S(g) + H2SO4 (l) -> 4H2O(l) + 4S (s) (yellow residue) (g)Reduces Hydrogen peroxide to water Experiment: (i)Pass a stream of Hydrogen sulphide gas in a test tu... | {
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Green solution Fe2+(aq) III. Brown solution Fe3+(aq) (c)Using acidified potassium dichromate(VI) describe how you would differentiate between sulphur(IV)Oxide and hydrogen sulphide -Bubble the gases in separate test tubes containing acidified Potassium dichromate(VI) solution. -Both changes the Orange colour of acidifi... | {
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The acid exist as a dibasic acid with two ionisable hydrogen. It forms therefore the Sulphate (VI) (SO42-) and hydrogen sulphate (VI) (HSO4-) salts. i.e. H2SO4 (aq) -> 2H+(aq) + SO42-(aq) H2SO4 (aq) -> H+(aq) + HSO4 -(aq) All Sulphate (VI) (SO42-) salts dissolve in water/are soluble except Calcium (II) sulphate (VI) (C... | {
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It forms therefore the Sulphate (IV) (SO32-) and hydrogen sulphate (VI) (HSO4-) salts. i.e. H2SO3 (aq) -> 2H+(aq) + SO32-(aq)
41 H2SO3 (aq) -> H+(aq) + HSO3 -(aq) All Sulphate (IV) (SO32-) salts dissolve in water/are soluble except Calcium (II) sulphate (IV) (CaSO3), Barium (II) sulphate (IV) (BaSO3) and Lead (II) sulp... | {
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Test any gases produced using litmus papers. Observations: -Colourless droplets of liquid forms on the cooler parts of the test tube in all cases. -White solid residue is left in case of Zinc (II)sulphate(VI),Sodium (I) sulphate (VI) and Sodium (I) sulphate (IV). -Colour changes from green to brown /yellow in case of I... | {
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Explanation (i)All Sulphate (VI) (SO42-) salts exist as hydrated salts with water of crystallization that condenses and collects on cooler parts of test tube as a colourless liquid on gentle heating. e.g. K2SO4.10H2O(s) -> K2SO4(s) + 10H2O(l) Na2SO4.10H2O(s) -> Na2SO4(s) + 10H2O(l) MgSO4.7H2O(s) -> MgSO4(s) + 7H2O(l) C... | {
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(ii) Copper(II)sulphate(VI) decomposes on strong heating to black copper (II) oxide and Sulphur (VI) oxide gas. Chemical equation 2CuSO4 (s) -> CuO(s) + SO3(g) This reaction is used for the school laboratory preparation of small amount of sulphur(VI)oxide gas. 6. The following experiments show the test for the presence... | {
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Observation 1 Observation Inference White precipitate/ppt persists SO42- , Cl- ions Observation 2 Observation Inference White precipitate/ppt dissolves SO32- , CO32- , ions III.(a)To the preserved sample observation 1 in (II) above, Heat to boil. Observation 1
43 Observation Inference White precipitate/ppt persists on ... | {
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To the preserved sample in (I) above, add six drops of 2M nitric(V) acid . Preserve. Observation 1 Observation Inference White precipitate/ppt persists SO42- , ions Observation 2
44 Observation Inference White precipitate/ppt dissolves SO32- , CO32- , ions III.To the preserved sample observation 2 in (II) above, add 4 ... | {
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Chemical/ionic equation: Pb2+(aq) + Cl- (aq) -> PbCl2(s) Pb2+(aq) + SO42+ (aq) -> PbSO4 (s) Pb2+(aq) + SO32+ (aq) -> PbSO3 (s) Pb2+(aq) + CO32+ (aq) -> PbCO3 (s) (ii)When the insoluble precipitates are acidified with nitric(V) acid, - Lead(II)chloride and Lead(II)sulphate(VI) do not react with the acid and thus their w... | {
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Chemical equation: 5SO32-(aq) + 2MnO4- (aq) +6H+(aq) -> 5SO42-(aq) + 2Mn2+(aq) + 3H2O(l) (purple) (colourless) 3SO32-(aq) + Cr2O72-(aq) +8H+(aq) -> 3SO42-(aq) + 2Cr3+(aq) + 4H2O(l) (Orange) (green) - Carbon(IV)oxide forms an insoluble white precipitate of calcium carbonate if three drops of lime water are added into th... | {
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46 Chemical/ionic equation: Ba2+(aq) + SO42+ (aq) -> BaSO4 (s) Ba2+(aq) + SO32+ (aq) -> BaSO3 (s) Ba2+(aq) + CO32+ (aq) -> BaCO3 (s) (ii)When the insoluble precipitates are acidified with nitric(V) acid, - Barium (II)sulphate(VI) do not react with the acid and thus its white precipitates remain/ persists. - Barium(II) ... | {
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Carbon(IV)oxide will not. Chemical equation: 5SO32-(aq) + 2MnO4- (aq) +6H+(aq) -> 5SO42-(aq) + 2Mn2+(aq) + 3H2O(l) (purple) (colourless) 3SO32-(aq) + Cr2O72-(aq) +8H+(aq) -> 3SO42-(aq) + 2Cr3+(aq) + 4H2O(l) (Orange) (green) - Carbon(IV)oxide forms an insoluble white precipitate of calcium carbonate if three drops of li... | {
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Sulphur(IV)oxide will not. Chemical equation: Ca(OH)2(aq) + CO2 (g) -> CaCO3(s) + H2O(l) These tests should be done immediately after acidifying to ensure the gases produced react with the oxidizing agents/lime water. 47 Summary test for Sulphate (VI) (SO42-)and Sulphate(IV) (SO32-) salts Practice revision question 1. ... | {
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Study the flow chart below and use it to answer the questions that follow Unknown salt Lead(II)nitrate(V) White precipitates of Cl-, SO42- , SO32- and CO32- Dilute nitric(V) acid white ppt dissolves in SO32- and CO32- white ppt persist /remains in SO32- and CO32- Acidified KMnO4 decolorized in SO32- White ppt with lime... | {
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Green solution from the orange solution 3SO32-(aq) + Cr2O72-(aq) +8H+(aq) -> 3SO42-(aq) + 2Cr3+(aq) + 4H2O(l) (Orange) (green) 2. Study the flow chart below and answer the questions that follow. 49 (i)Write equation for the reaction taking place at: I.The roasting furnace (1mk) 2FeS2 (s) + 5O2 (g) -> 2FeO(s) + 4SO2 (g)... | {
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49 (i)Write equation for the reaction taking place at: I.The roasting furnace (1mk) 2FeS2 (s) + 5O2 (g) -> 2FeO(s) + 4SO2 (g) II.The absorption tower (1mk) H2SO4 (l) + SO3 (g) -> H2S2O7(l) III.The diluter (1mk) H2S2O7(l) + H2 O(l) -> 2H2SO4 (l) (ii)The reaction taking place in chamber K is SO2 (g) + 1/2O2 (g) SO3 (g) I... | {
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Explain why it is necessary to use excess air in chamber K To ensure all the SO2 reacts II.Name another substance used in chamber K Vanadium(V)oxide 3.(a)Describe a chemical test that can be used to differentiate between sodium sulphate (IV) and sodium sulphate (VI). Add acidified Barium nitrate(V)/chloride. White prec... | {
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Add acidified Barium nitrate(V)/chloride.
White precipitate formed with sodium sulphate (VI) No white precipitate formed with sodium sulphate (IV) (b)Calculate the volume of sulphur (IV) oxide formed when 120 kg of copper is reacted with excess concentrated sulphuric(VI)acid.(Cu = 63.5 ,1 mole of a gas at s.t.p =22.4d... | {
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